CHM 130LL: The Metric System - Glendale Community College

CHM 130LL: The Metric System

In this experiment you will: Determine the volume of a drop of water using a graduated cylinder

Determine the volume of an object by measuring its dimensions

Determine the volume of an object using volume by displacement

Measure the mass of various objects using an analytical balance Learn how to use a burette to dispense a liquid Practice conversions using English and metric units

In the U.S., the English system of measurement is used almost exclusively. For example, the fuel efficiency of a car is reported in miles per gallon; a person's height is usually given in feet and inches; ice cream is sold by the cup, pint or gallon; one's weight is measured in pounds, and temperature is reported in degrees Fahrenheit. However, the English system can be quite complex when it comes to conversions. For example, few people can remember that one mile equals 5280 feet or 1760 yards.

A much more effective system uses a decimal system of measurement, where basic units are used in conjunction with prefixes to represent multiple or fractions of the base unit. The metric system is such a system. For example, in the metric system, the base unit for mass is the gram. A multiple of the base unit can be expressed by combining a metric prefix, like kilo representing 1000, with the base unit to give the unit kilogram, which equals 1000 grams.

Because of its logic and simplicity, the metric system gained international acceptance with the Treaty of the Meter, establishing the International Bureau of Weights and Measures. Even the United States signed the treaty in 1875, but to date the U.S.'s use of the metric system seems to be the limited to 2-liter bottles for soda and cc's (cubic centimeters) in hospitals. In science, the metric system is used almost exclusively, so most of the equipment and instruments used in a chemistry lab generally measure centimeters, millimeters, milliliters, and grams.

In this experiment, you will learn how to use a variety of chemistry laboratory equipment and instruments to become more familiar with the metric system. You will use graduated cylinders to measure volume, an analytical balance to measure mass, and a ruler to measure the length, width, and height of a rectangular solid.

You will also learn about a method called volume by displacement, where the volume of an object is determined using the volume of water displaced. You will also use mass by difference to determine the mass of a sample.

Finally, you will practice determining the number of significant figures for each measurement and expressing the answers for calculated measurements with the

4

correct number of significant figures.

Laboratory Techniques

Graduated cylinders are used to contain and deliver measured amounts of liquid. They are available in many sizes. You will use the 10 mL and 100 mL sizes. Always use the smallest graduated cylinder that will hold the entire volume. The 10-mL graduated cylinders are always read to 2 decimal places (e.g. 5.50 mL) and the 100-mL graduated cylinders are always read to 1 decimal place (e.g. 50.5 mL).

When water is placed in a glass cylinder, a concave surface forms; this curve is called the meniscus. Glass graduated cylinders are manufactured

GCC CHM 130LL: Introduction to the Metric System

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2.77 mL

2

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so that the line at the bottom of the meniscus gives the most accurate reading. In order to read any graduated cylinder accurately, it must be level (sitting on the counter, NOT hand-held). Your eye must also be perpendicular to the water level. Note that the graduations on all cylinders rise from the bottom up. That is, they indicate the volume contained in the cylinder.

The 10-mL graduated cylinder above is read to two decimal places (to the nearest 0.01 mL). Thus, the volume of liquid is read to be 2.77 mL.

Note that 100-mL graduated cylinders have markings for each mL, so they are read to one decimal place (to the nearest 0.1 mL).

Rulers: The basic metric unit of length is the meter, but the length of most objects in a chemistry lab are

measured

in centimeters

(cm).

A centimeter

equals

0.01m or

1 100

of

a

meter,

so

1m

100cm

just

like

1

dollar

100 cents (since one cent is equal to

1 100

of a dollar).

Several instruments are used for metric length measurements, such as a centimeter ruler in the example below. The numbers shown on a centimeter ruler are centimeters (cm), and the 10 smaller markings between each

number represent millimeters (mm). (Note that 10mm 1cm.) When measuring, always place an object at the "0" mark.

Consider the stick and ruler below:

0

1

2

When taking a measurement, all the digits are known with certainty, except the last digit, which is estimated. If the object appears to be exactly on a marking, then the estimated digit is 0. If the object appears to be exactly halfway between two markings, the estimated digit is 5. The stick above appears to be a little past the halfway point between 1.2 and 1.3, so its length is recorded as 1.27 cm.

Balances: In most chemistry labs, balances are used to determine the mass of a sample. The metric unit of mass is the gram. You will use electronic balances. These balances are very expensive, very sensitive and must be used very carefully to avoid damage. The general procedure follows. The most important rule is NEVER place any chemical directly on the balance pan. Use a beaker, a watch glass, a plastic weighing cup, or weighing paper.

The balances are to remain "ON" at all times.

All doors or lids are to remain closed at all times, except when loading or unloading the balance. Note the balanced in PS 155 do not have doors!

Do not lean on the balance table. (The balance is sensitve enough to measure vibrations on the countertop due to students leaning on it.)

Material to be weighed should be placed in a container on the balance pan. The container may be either pre-weighed or "tared" or zeroed out (as explained later).

Before weighing, be sure the doors/lid are closed and the digital scale reads all zeros. If zeroes are not displayed on the scale, gently click the front lever until the balance displays zeros. If 0.00000 g (5 zeros

past decimal) is displayed or if the number displayed continues to drift, consult your instructor.

To weigh an item, open the door, and carefully place the item on the center of the pan. Close the door and wait for the digital readout to stabilize (the green light to the left of the readout will go off). Read and record all the numbers in the digital readout. (Never round any numbers reported on any electronic instrument.) Remove the item and close the doors/lid before leaving.

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 If you are using a container to hold chemicals, you may tare or zero the container. To do that, place the container carefully in the center of the pan. Close the doors. Briefly click on the left of the front lever (as in zeroing the balance). Zeros should appear. The container is now "tared out," and the balance is set to read the weight of any material added to the container. Remove the container from the balance, add material to it, and carefully place the container back on the center of the pan. (Do NOT re-zero the balance during this process.) Close the door and read the digital scale when stabilized as before. After you have removed the container, shut the doors and gently push the front lever to remove the tare and return the scale to zero.

Significant Figures (Sig figs)

Rules 1. Digits 1 through 9 are always significant. (347 has 3 sig figs) 2. Zeroes in front are never significant. (0.00024 has 2 sig figs) 3. Zeroes in between significant digits are always significant. (7030 has 3 sig figs) 4. Zeroes after a number are significant if they are ALSO after a decimal place. (0.3500 has 4 sig figs)

Addition and subtraction ? the answer has the same number of decimal places as the least decimal places in the calculation. (24.6 ? 9.2456 = 15.4 because the answer must have one decimal place)

Multiplication and division ? the answer has the same number of significant digits as the least significant number in the calculation. (42 x 4378 = 180,000 because the answer must have two sig figs)

Procedure

A. INVESTIGATING MASS

1. Review the instructions in the Laboratory Techniques section for using the electronic balances.

2. In the plastic shoebox-size container at your lab station, you will find various objects. Use the electronic balance to measure the mass of each of the following objects: a small paper clip, a large paper clip, the cap of a ballpoint pen, and one sheet of paper (folded 4 times to fit on the balance pan). Be sure to place each object near the center of the balance pan to weigh it. Record the mass of each object by writing down all the numbers, as displayed by the balance. NEVER round the mass reported on an electronic balance!

3. Indicate the number of significant figures for each mass measurement, then answer the questions at the end of Part A on the Lab Report form.

B. INVESTIGATING LENGTH AND VOLUME

1. Review the instructions in the Laboratory Techniques section for using centimeter rulers. Be sure to use the side with markings in centimeters and millimeters (not inches).

2. Measure the length, width, and height of the rectangular metal solid. Record each dimension in centimeters (to 2 decimal places). The little lines are millimeters by the way.

3. Answer the questions on length and significant figures. Calculate the volume of the rectangular object using the formula below. Be sure to record the volume with the correct units.

volume = length width height

4. Review the instructions in the Laboratory Techniques section for using graduated cylinders.

5. Obtain about 50 mL of tap water in your 150-mL beaker using the markings on the beaker. Pour the water from the beaker to your 100-mL graduated cylinder to about the 40-mL mark. Record the exact volume of water in the graduated cylinder (to 1 decimal place).

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6. Tilt the graduated cylinder until it is at an angle, and carefully lower the rectangular solid so as not to splash any water out of the graduated cylinder. Slowly return the graduated cylinder to an upright position to avoid the metal piece hitting and breaking the glass bottom of the graduated cylinder. Read and record the exact new volume of water (to 1 decimal place).

7. Subtract the original volume of water from the final volume of water, and record the difference (to 1 decimal place) with the appropriate units.

8. Compare the two volumes determined for the rectangular object, and answer the questions at the end of Part B.

C. INVESTIGATING DI WATER

1. Review the instructions in the Laboratory Techniques section for using Balances, particularly the section on how to "Tare" or Re-Zero the Balance.

2. Obtain about 20 mL of deionized (DI) water in your 50-mL beaker using the markings on the beaker.

3. Carefully place a dry plastic weighing cup in the center of the pan in an analytical balance. Tare (or re-zero) the balance. The display should now read all zeroes.

4. Carefully remove the plastic weighing cup. Use a disposable pipet to add one drop of water into the plastic weighing cup. Return the cup to the balance, and record the mass of one drop of water.

5. Review the instructions in the Laboratory Techniques section for using graduated cylinders.

6. Use a disposable pipet to add DI water to your 10-mL graduated cylinder exactly to the 4.00 mL mark. The pipet is in your tub, put it back in your tub when done.

7. Make sure the outside of the graduated cylinder is completely dry, make sure the empty balance says 0.0000, then measure and record the mass of the graduated cylinder with 4.00 mL of DI water.

8. Next, you will determine the number of drops of water in one milliliter by carefully counting the number of drops required to raise the water level in the graduated cylinder to the 5.00 mL mark. Record the number of drops of water used to get to the 5.00 mL mark (i.e., the number of drops equal to 1.00 mL).

9. Measure and record the mass of the graduated cylinder with 5.00 mL of DI water.

10. Subtract the initial mass (graduated cylinder + 4.00 mL DI water) from the new mass (graduated cylinder + 5.00 mL DI water) to get the mass of 1.00 mL of DI water. Record the difference with the appropriate units.

11. Calculate the number of drops of water in 1.00 mL by dividing the mass of 1.00 mL of DI water by the mass of one drop of water. Compare your answer with your experimentally determined number of drops from step 8 above.

D. INVESTIGATING HOW A BURETTE DISPENSES WATER

Burettes are used to measure the amount of liquid delivered. So instead of measuring how much liquid is inside the burette, you actually measure how much liquid comes out of the burette into a second container. Burettes are very expensive due to their good accuracy. Do not break your burette.

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1. Obtain a burette from the instructor cart. Be careful, if you break it, you buy it! Clamp your burette to the ring stand with the burette clamp.

2. Put your funnel in the top of the burette. Put approximately 20 mL of water into your 50 mL beaker. Now pour all the water into the burette. Allow the tip of the burette to fill by draining a small amount out of the burette into your beaker. Now record the burette reading as your initial burette volume to 2 decimal places.

3. Empty and dry your 50 mL beaker. Go and weigh the empty beaker. Record the mass for the empty dry 50 mL beaker.

4. Now dispense approximately 12 mL from the burette into the clean dry 50 mL beaker. Record the final volume of the burette as final burette volume to 2 decimal places.

5. Go and weigh the 50 ml beaker again with the water in it. Record the mass for the 50 mL beaker plus water.

6. Calculate the amount dispensed from the burette by subtracting the initial volume from the final volume of the burette. Record as the volume of water dispensed.

7. Calculate the mass of the water by subtracting the mass of the empty 50 mL beaker from the 50 mL beaker plus water. Record as mass of water.

8. Calculate the density of the water by dividing the mass of water by the volume of the water dispensed.

9. The density of water is close to 1.00 g/mL. Compare this to your density. Why might they be different?

Put everything back where you found it. Wipe up any spills. Wash your hands and your bench.

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